So I posted this question yesterday and was told I had a few typos.... I fixed them and here is the question again... Please help me!!!

A solution of ferrous sulfate (FeSO4) is titrated with a solution of potassium permanganate in sulfuric acid. The balanced half reactions are as follows:

10FeSO4 + 5 H2SO4 --> 5 Fe2(SO4)3 + 10 H ^+ +10e^-
and 2 KMnO4 + 3 H2SO4 +10e^- --> 2 MnSO4 + K2SO4 + 8 H2O.

The gram-formula mass of FeSO4 is 151.91 g/mol, and that of KMnO4 is 158.04 g/mol.

1. What is the gram-equavalent mass of FeSo4 for this reaction?

2. What is the gram-equavalent mass of KMnO4 for this reaction?

3. If 5.35 g of KMnO4 are dissolved in
a liter of solution, what is the normality of the solution?

4. If 65.34 mL of 0.1000 N KMnO4 are required to titrate 45.28 mL of FeSO4 solution, what is the normality of the solution?

5. Carbon monoxide is detected in air samples by its reaction with diiodine pentoxide to form carbon dioxide and elemental iodine: CO + I2O5 --> CO2 + I2. Balance the equation.

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  1. my answers so far...

    1. 151.91g FeSO4/1eq

    2. 31.608g KMnO4/1eq

    3. N=5eq/1L (not sure about this one)

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